Acompressor takes 0.50 m3 of a gas at 33°c and 760 mmhg and compresses it to 0.10 m3, cooling it to -55°c at the same time. what is the pressure of the gas at these new conditions? 3.7 x 10-4 mmhg 68 mmhg 2,700 mmhg 1.0 mmhg

2,700 mmHg.

Explanation:

where, P is the pressure of the gas in atm.

V is the volume of the gas in L.

n is the no. of moles of the gas in mol.

R is the general gas constant,

T is the temperature of the gas in K.

P₁V₁T₂ = P₂V₂T₁

P₁ = 760 mmHg, V₁ = 0.50 m³, T₁ = 33°C + 273 = 306.0 K.

P₂ = ??? mmHg, V₂ = 0.10 m³, T₂ = - 55°C + 273 = 218.0 K.

∴ P₂ = P₁V₁T₂/V₂T₁ = (760 mmHg)(0.50 m³)(218.0 K)/(0.10 m³)(306.0 K) = 2707.0 mmHg ≅  2,700 mmHg.

calculate how many grams of ammonia can be produced from 4.21 grams of

n2 + 3h2 = 2nh3

my answer:

25.0g n2 x (1 mol/ 28.0gn2) x (2 mol nh3/ 1 mol n2) x (17.0g nh3/ 1 molnh3) = 30.36g n2

25.0g h2 x (1 mol h2/ 2.00g h2) x (2 mol nh3/ 3 mol h2) x (17.0g nh3/ 1 mol nh3) = 141.67g h2

lr = n2

c (diamond),

sio2 (quartz)