Calculate the amount of H2S required to react completely with 11.3dm^3 of SO2 at S.T.P....

Calculate the amount of H2S required to react completely with 11.3dm^3 of SO2 at S.T.P. The equation for the reaction is
2H2S+SO2→2H2O + 3S. One mole of a gas occupies 22.4dm at S.T.P?

In Chemistry
1 Answers Available
Asked by Adaora on 18th April, 2018

NECO June/July 2024 - Get offline past questions & answers - Download objective & theory, all in one app 48789

Post-UTME Past Questions - Original materials are available here - Download PDF for your school of choice + 1 year SMS alerts

To get notifications when anyone posts a new answer to this question,
Follow New Answers

Answers ({{ comment_count }})

Please wait...

{{ settings.no_comment_msg ? settings.no_comment_msg : 'There are no comments' }}

Ask Your Own Question

Quick Questions

1.Define chemical industry 2.List and explain types of chemical.? Answer this

1 Answers · Chemistry · 3 days ago
a student was asked to electroplate a stainless steel spoon using a brass rod has the electrode and copper 2... Answer this

1 Answers · Chemistry · 3 days ago
A hydrocarbon with a vapor density of 29 contains 82.76% carbon and 17.24% hydrogen. Determine the empirical formula? Answer this

1 Answers · Chemistry · 4 days ago

See More Chemistry Questions

Calculate the amount of H2S required to react completely with 11.3dm^3 of SO2 at S.T.P....

Post an Answer

Answers ({{ comment_count }})

Please wait...

Modal title

Report

Block User

{{ feedback_modal_data.title }}

Quick Questions

Sign In