Suppose that 5.14 x 10-3 mol of hydrogen gas occupies a 1,171 ml container at 60°c. what is the pressure (in torr)? (do not type the units.)

Explanation:

Given that:

Temperature = 60 °C

The conversion of T( °C) to T(K) is shown below:

T(K) = T( °C) + 273.15  

So,  

T₁ = (60 + 273.15) K = 333.15 K  

n = 5.14 × 10⁻³ mol

V = 1,171 mL = 1.171 L ( 1 mL = 0.001 L)

Using ideal gas equation as:

where,  

P is the pressure

V is the volume

n is the number of moles

T is the temperature  

R is Gas constant having value = 62.364 L Torr/ K mol  

Applying the equation as:

P × 1.171 L = 5.14 × 10⁻³ mol × 62.364 L Torr/ K mol  × 333.15 K  

⇒P = 91.2 torr

1)Reaction of strong base and acidic salt

2)Reaction of acid and base

Explanation:

1)  Ammonium carbonate is basically a acidic salt in nature. When it comes in contact of strong base it behave as strong acid and dissociate. Ammonium ion give i's H+ to NaOH and release ammonia gas and water. H2O react with left carbonate ion to form sodium carbonate.

2)  Phosphoric acid is tri basic acid and calcium hydroxide is a base and reacts to form salt and water as side product.