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calculate the amount of thermal energy associated with 80 g of ice at 0 degrees celsius turning into water at 0 degrees celsius. (mm of H20= 18.02 g/mol, Heat of fusion (water)= 6.02 kJ/mol).

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Calculate the amount of thermal energy associated with 80 g of ice at 0

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Given that Q Total is 100.3252kJ of H2O from a solid at -50°C to a vapour at 230°C, prove that the specific heat of water is 4.18J/ (gx°C). Validate your answer and explain your thinking.
This is given that:
Latent heat of fusion is 6.01kJ/mol
Latent heat of vaporisation is 40.7kj/mol
Specific heat of ice is 2.1J/ (gx°C)
Specific heat of vapour is 1.7J/ (gx°C)

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If 2.00 mol of H2 and 3.00 mol of I2 are placed in a 1.00 L vessel at 1100K, what is the concentration of each gas at equilibrium?

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Calculate the amount of heat energy required to convert 98.50g of vapour (at 250) to solid water (ice at -80) Boiling point of water 100 degrees and freezing point is 0 degrees. the molar heat of condensation and fusion of water are 40.7 kj/mol and 6.01kj/mol respectively . The specific heat of vapour, liquid and solid are 1.7J, 4.18J and 2.1J respectively

Clearly label and sketch the process, explain and compare why there is no temperature increase during the process of condensation and fusion

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Apply Hess's Law to calculate the change in enthalpy for the given reaction and justify your answer with a statement:

CS₂(ℓ) + 3O₂(g) ---> CO₂(g) + 2SO₂(g) = 1229.5kJ
Given:

C(s) + O₂(g) ---> CO₂(g) | ΔH = at the bottom
S(s) + O₂(g) ---> SO₂(g) | ΔH =
C(s) + 2S(s) ---> CS₂(ℓ) | ΔH =

1. 1229.5KJ
2. -787KJ
3. -285.8KJ

or
Apply the quadratic formula and expression to find the concentration of the aqueous solutions of 2.00mol of HCL, 1.00 mol of Na2 which produces 1.00 mol of H2 and 2.00mol of NaCl. Show all methods and justify your answer with a statement.

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The total amount of heat energy required to convert 140.25g of solid water (ice) at -45 degrees C to water is 43.68kJ. (The melting and boiling points of water are 0 degrees C and 100 degrees C respectively, the molar heats of fusion ad vaporisation of water are 4.76kJ/mol and 36.2kJ/mol respectively. The specific heats of water in the solid, liquid and vapour forms are 1.9J/g.C, 4.18J/g.C and 2.1J/g.C respectively.)

Calculate the final temperature of the water when this amount of heat energy is applied. Clearly outline each step of the working and reasoning used to obtain your answer. Also include appropriate and well labeled sketches/graphs/diagrams in your response. Be sure to explain the relevant trends and patterns in the data.

**HINT **  molar mass  = 18.01528

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The total amount of heat energy required to convert 140.25g of solid water (ice) to vapour (at 349.99°C) is 499.77kJ. (The melting and boiling points of water are 0°C and 100°C respectively and the molar heats of fusion and vaporisation of water are 6.01 kJ/mol and 40.7kJ/mol respectively. The specific heats of water in the solid, liquid and vapour forms are 2.1J/(gx°C), 4.18J/(gx°C) and 1.7J/(gx°C) respectively.)

Calculate the initial temperature of the solid water, when this amount of heat energy is required to convert it to a vapour at 100.25°C.

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Calculate the total amount of energy required to to convert gaseous water (vapour) at 275.34 degrees celsius down to water at -11.2 degrees celsius. The melting and boiling points of water are 0°C and 100°C respectively and the molar heats of fusion and vaporisation of water are 6.01 kJ/mol and 40.7 kJ/mol respectively.  The specific heats of water in the solid, liquid and vapour forms are 2.1 J/(gx°C), 4.18 J/(gx°C) and 1.7 J/(gx°C) respectively.). Determine the amount of energy absorbed or given off to go from 275.34 degrees celsius down to -11.2 degrees celsius for water. Draw graphs and identify trends.

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1)    Evaluate the amount heat energy required for 1543.235835294 calories of solid water (ice) (at 183.15K) to determine how much energy in total is required to begin melting the ice. (The melting points of water are 0°C and the molar heat of fusion is 6.01kJ/mol respectively.  The specific heat of water in the solid form is 2.1 J/ (gx°C).) Further: explore, explain and evaluate the difference in the amount of heat required in the ice (water solid) compared to the amount of energy needed to convert 2314.853752941 calories of sodium (solid) at -226.85 K to the point it starts melting. (The molar heat of fusion for sodium is 97.42kJ/mol respectively. The specific heat of Na in the solid form is 1.23 J/ (gx°C) respectively.)

Include appropriate and well-labelled sketches/graphs/diagrams in your response, as well as explain any trend and patterns in the data to justify your results.

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Remember it asks to sketch and explain the trends and patterns

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Q1 or Q2
Test you would be given specific heats, and heat of fus and vap

Varied units.
Find c
Finding starting temp
Finding final temp
Reverse going from Vapour to Solid

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Miss Bamford's Question

Calculate the amount of heat energy required to convert 150.45 g of solid water (ice) (at -80°C) to water vapour at 250°C.  (The melting and boiling points of water are 0°C and 100°C respectively and the molar heats of fusion and vaporisation of water are 6.01 kJ/mol and 40.7 kJ/mol respectively.  The specific heats of water in the solid, liquid and vapour forms are 2.1 J/(gx°C), 4.18 J/(gx°C) and 1.7 J/(gx°C) respectively.)

Clearly outline each step of the working and reasoning used to obtain your answer.  Also include appropriate and well-labelled sketches/graphs/diagrams in your response.   Be sure to FULLY explain any relevant trends or patterns in the data.

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Remember
Understand
Apply
Analyse
Evaluate
Explore
Compare
Explain
Justify