A sample of hydrogen gas has a volume of 8560. mL at standard temperature and a pressure
of 1.50 atm. Calculate the number of moles of H, present in this gas sample.

5.26 moles

Explanation:

Given that:

Volume of hydrogen gas V = 8560mL

(since 1000 mL = 1dm3

8560mL = 8560/1000= 8.56dm3)

Standard temperature T = 25°C

Convert temperature in Celsius to Kelvin

(25°C + 273 = 298K)

Pressure P = 1.5atm

Number of moles of hydrogen = ?

Note that Molar gas constant R is a constant with a value of 0.0082 ATM dm3 K-1 mol-1

Then, apply ideal gas equation

pV = nRT

1.5 atm x 8.56dm3 = n x (0.0082 atm dm3 K-1 mol-1 x 298K)

12.84atm dm3 = n x 2.44atm dm3 mol-1

n = (12.84atm dm3 / 2.44atm dm3 mol-1)

n = 5.26 moles

Thus, there are 5.26 moles of Hydrogen, H present in this gas sample.

1.consider the following balanced equation and answer parts a through. show calculations for each part.  

3 ag(s) + 4 hno3(aq) → 3 agno3(aq) + no(g) + 2 h2o(l)  

a. calculate the number of moles of agno3 produced by the reaction of 3 moles of ag with excess hno3. if the number to the left of the compound represents the number of moles of the compound which are present, then 3 moles of ag react with 4 moles hno3 to produce 3 moles agno3 (aq).

so the answer to a would be 3 moles.

b. calculate the number of moles of agno3 produced by the reaction of 108 grams of ag with excess hno3.  

i'm not sure how to plug in the grams of silver into an equation using moles to find how many moles are produced.

c. calculate the number of grams of agno3 produced by the reaction of 108 grams of ag with excess hno3  

d. calculate the number of moles of no produced as a byproduct of the reaction of 108 grams of ag with excess hno3.  

e. calculate the number of grams of no produced as a byproduct starting with 108 grams of ag and excess hno3.  

explanation:

it should be all of them because it asks if you included all of those in your answer

explanation: