1. Questions

chemistry

1. Given that 50 grams of ice is heated at -20.0 °C to steam at 135.0 °C.
i. Show the graph of the changes from ice to steam
ii. Calculate the energy needed to change the ice to steam
Please use these values:
Heat of fusion = 334.16 J g¯1
Heat of vaporization = 2259 J g¯1
specific heat capacity for solid water (ice) = 2.06 J g¯1 K¯1
specific heat capacity for liquid water = 4.184 J g¯1 K¯1
specific heat capacity for gaseous water (steam) = 2.02 J g¯1K¯1

  1. 👍
  2. 👎
  3. 👁
bliss

  1. q1 = heat needed to raise T ice froom -20 to zero C.
    q1 = mass ice x specific heat ice x (Tfinal-Tinitial)

    q2 = heat needed to melt ice @ zero C to liquid water @ zero C.
    q2 = mass ice x heat fusion ice.

    q3 = heat needed to raise T water at zero to 100 C.
    q3 = mass water x specific heat H2O x (Tfinal-Tinitial)

    q4 = heat needed to convert water @ 100 C to steam at 100 C.
    q4 = mass water x heat vaporization

    q5 = heat needed to raise T of steam at 100 to steam at 135.
    q5 = mass steam x specific heat steam x (Tfinal-Tinitial)

    Total q = q1 + q2 + q3 + q4 + q5

    1. 👍
    2. 👎
    DrBob222

  2. 33kj

    1. 👍
    2. 👎
    Anonymous

Respond to this Question

First Name

Your Response

Similar Questions

  1. Chemistry

    Calculate the amount of energy in kilojoules needed to change 225 g of water ice at -10 C to steam at 125 C. The following constants may be useful: Cm(ice)=36.57 J/(mol*C) Cm(water)=75.40 J/(mol*C) Cm(steam)=36.04 J/(mol*C) Delta

  2. Chemistry

    How much heat (in kilojoules) is required to warm 11.0 g of ice, initially at -14.0 ∘C, to steam at 112 ∘C? The heat capacity of ice is 2.09 Jg−1∘C−1 and that of steam is 2.01 Jg−1∘C−1.

  3. Science

    Find out the amount of heat required to convert 1 gm of ice at -30 ⁰C to 1 gm of steam at 120 ⁰C. Given the specific heat of ice is 2090 J/kg/⁰C, specific heat of water 4180 J/kg/⁰C, specific heat of steam is 2010

  4. Chemistry

    How many grams of ice could be melted by the energy obtained as 18.0 grams of steam is condensed at 100.0 degrees celcius and cooled to 0.0 degrees celcius?

  1. Physics

    How much heat is added to a 10.0 g of ice at -20.0 degrees Celsius to convert it to steam at 120.0 degrees Celsius? compute and add the following heats: heat to heat ice from -20C to 0C heat to melt ice at 0C Heat to heat water

  2. Chemistry

    How much energy does it take to convert 0.800 kg ice at -20.°C to steam at 250.°C? Specific heat capacities: ice, 2.1 J g-1 °C-1 liquid, 4.2 J g-1 °C-1 steam, 2.0 J g-1 °C-1 ΔHvap = 40.7 kJ/mol, ΔHfus = 6.02 kJ/mol This is

  3. physics

    calculate the heat energy needed to convert 2kg of ice at -12 degree celcius to steam at 100 degree celcius. specific heat capacity for ice=2100j/kg K specific latent heat of ice=340000 J/kg specific latent heat for steam

  4. Chemistry

    Topic: Sublimation and Fusion How much heat (in kJ) is required to warm 13.0 g of ice, initially at -14.0 C, to steam at 112.0 °C? The heat capacity of ice is 2.09 J/g⋅°C and that of steam is 2.01 J/g⋅°C. Any help on how to

  1. chemistry

    how much heat (in KJ) is evolved in coverting 1.00 mol of steam at 135.0 degrees celcius to ice at -45.0 degrees celcius? the heat capacity of steam is 12.0 J/g * C and ice is 2.09 J/c * C.

  2. chemistry

    Calculate the enthalpy change (in kJ) associated with the conversion of 25.0 grams of ice at -4.00 °C to water vapor at 109.0 °C. The specific heats of ice, water, and steam are 2.09 J/g-K, 4.18 J/g-K, and 1.84 J/g-K,

  3. general chemistry

    Calculate the total amount of heat absorbed (in kJ) when 2.00 mol of ice at -30.0°C is converted to steam at 140.0°C. (Cp(ice)=2.06 J/g∘C; Cp(water)=4.18 J/g∘C; Cp(steam)=1.87 J/g∘C) (7 pts: Given-1point; Formula-1point;

  4. Physics

    How much energy is required to change a 58 g ice cube from ice at −1◦C to steam at 101◦C? The specific heat of ice is 2090 J/kg ·◦ C and of water 4186 J/kg ·◦ C. The latent heat of fusion of water is 3.33 × 105 J/kg,

You can view more similar questions or ask a new question.