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

i think its 5049.

i hope this !

ca has a crystalline lattice with positive ions (since it is a metal, metals are positively charged) and electrons flow freely in its structure since the ca atoms have a large nuclear radius so the electrons are not tightly held, therefore the electrons can flow freely since they are not being highly attracted by the nucleus. moreover, one of the properties of metals are that they are conductors of electricity, thus proving ca is the element.