There is 50.0 ml of a gas at a temperature of 5°c. its pressure is 760 mm hg. what temperature is needed
to change the volume to 55ml and the pressure to 780 mm hg?

41°C

Explanation:

Ideal gas law:

PV = nRT

where P is absolute pressure,

V is volume,

n is number of moles,

R is universal gas constant,

and T is absolute temperature.

n is held constant, so:

P₁V₁ / T₁ = P₂V₂ / T₂

Given:

P₁ = 760 mmHg

V₁ = 50.0 mL

T₁ = 5°C = 278 K

P₂ = 780 mmHg

V₂ = 55 mL

Find: T₂

(760 mmHg) (50.0 mL) / (278 K) = (780 mmHg) (55 mL) / T

T = 314 K

T = 41°C

answer: 802.3 kilo joules of energy represents 191.75 kilo calorie of energy.

explanation:

energy released during combustion of one mole methane = 802.3 kilo joules

if 1 kilo joule = 0.239006   kilo calorie

then ,802.3 kilo joule will be = 802.30.239006 kilo calorie

802.3 kilo joule = 191.75 kilo calorie

hence, the energy in kilo calorie is 191.75 kilo calorie.