4. When 732 grams of water was heated, it absorbed 1962 Joules of heat. The original temperature of the water was 45°C. What was the final temperature?

=final temperature

Explanation:

In the question specific heat of water is not given but we should know the value of that and it 4.18Jg∘C

Specific heat means how much heat is required to increase the temperature of 1 gram of substance that substance by 1∘C .

Equation between heat lost or gain and the change in temperature.

q=m⋅c⋅ΔT , where

q - the amount of heat

m - the mass of the sample

c - specific heat  of sample

ΔT - change in temperature

put all the given value into this ,

=final temperature.

in the given question, the partial pressure is calculated by using the ideal gas equation, that is, pv = nrt

here, p is pressure, v is volume = 25 l, n is number of moles = 0.0104 moles, r is gas constant = -0.0821 l.atm / mol.k

t is temperature = 273 k

p = nrt / v

p = (0.0104 mol × 0.0821 l.atm / mol.k × 273 k) / 25 l

= 0.0093 atm