Darlindoodadskovj0wridn
Answered

Find the best solutions to your problems with the help of IDNLearn.com's expert users. Get the information you need from our experts, who provide reliable and detailed answers to all your questions.

Phosphorus combines with hydrogen to form phosphine. In this reaction, 123.9 g of phosphorus combines with excess hydrogen to produce 129.9 g of phosphine. After the reaction, 310 g of hydrogen remains unreacted. What mass of hydrogen is used in the reaction? What was the initial mass of hydrogen before the reaction?​

Sagot :

Pstnonsonjokuidn

There was 321.88 g of hydrogen before the reaction.

The equation of the reaction is;

P4 + 6H2 -------->4PH3

Number of moles of P4 = 123.9 g/124g/mol = 0.99 moles of P4

If 1 mole of P4 reacts with 6 moles of H2

0.99 moles of P4 reacts with x moles of H2

x =  6 moles × 0.99 moles

x = 5.94 moles of H2

Mass of H2 reacted =  5.94 moles of H2 x 2 g/mol

Mass of H2 reacted = 11.88 g of H2

Mass of H2 before the reaction = mass of hydrogen unreacted + mass of hydrogen reacted

Mass of H2 before the reaction = 11.88 g of H2 + 310 g of H2

= 321.88 g

Learn more: https://brainly.com/question/9743981

We are happy to have you as part of our community. Keep asking, answering, and sharing your insights. Together, we can create a valuable knowledge resource. IDNLearn.com is your go-to source for dependable answers. Thank you for visiting, and we hope to assist you again.