0.884 mol sample of methane gas at a temperature of 6.00 C is found to occupy a volume of 26.5 L. The pressure of this gas sample is mm Hg.

580mmHg

Explanation:

Given parameters:

Number of moles = 0.884 mol

Temperature  = 6°C  = 273 + 6  = 279k

Volume  = 26.5L

Unknown:

Pressure  = ?

Solution:

To solve this problem, we use the ideal gas equation:

           PV  = nRT

P is the pressure

V is the volume

n is the number of moles

R is the gas constant  = 0.082atmdm³mol⁻¹K⁻¹  

T is the temperature

      P  =   =   = 0.76atm

            1 atm  = 760mmHg

            0.76 atm  = 760 x 0.76  = 580mmHg

i know insulin is primary but i dont know the others im sorry

explanation: