A 826.76 g sample of BrCl is in a 6342.7 mL container. What is the pressure of this gas in torr at 325.77 °C?

55.5atm

Explanation:

Using ideal gas law equation;

PV = nRT

Where;

P = pressure (atm)

V = volume (L)

n = number of moles (mol)

R = gas law constant (0.0821 Latm/molK)

T = temperature (K)

Molar mass of BrCl = 79.9 + 35.5

= 115.4g/mol

* mole = 826.76 g ÷ 115.4g/mol

mole = 7.16mol

* Volume = 6342.7 mL = 6342.7/1000 = 6.3427L

* Pressure = ?

* Temperature = 325.77 °C = 325.77 + 273 = 598.77K

PV = nRT

P = nRT/V

P = (7.16 × 0.0821 × 598.77) ÷ (6.3427)

P = 351.98 ÷ 6.3427

P = 55.5atm

n2(g) + 3h2-> 2nh3(g)   this is the balanced equation

note the mole ratio between n2, h2 and nh3.   it is 1 : 3 : 2   this will be important.

moles n2 present = 28.0 g n2 x 1 mole n2/28 g = 1 mole n2 present

moles h2 present = 25.0 g h2 x 1 mole h2/2 g = 12.5 moles h2 present

based on mole ratio, n2 is limiting in this situation because there is more than enough h2 but not enough n2.

moles nh3 that can be produced = 1 mole n2 x 2 moles nh3/mole n2 = 2 moles nh3 can be produced

grams of nh3 that can be produced = 2 moles nh3 x 17 g/mole = 34 grams of nh3 can be produced

note:   the key to this problem is recognizing that n2 is limiting, and therefore limits how much nh3 can be produced.

the correct answer is option d

explanation:

i was wrong its d because they dont use cm when calculating square roots