Asked by Lance
A sample of cesium metal reacted completely with water, evolving 48.7 mL of dry H2 at 24°C and 774 mmHg. What is the equation for the reaction? (Include states-of-matter under SATP conditions in your answer. Use the lowest possible coefficients.)
What was the mass of cesium in the sample?
What was the mass of cesium in the sample?
Answers
Answered by
DrBob222
2Cs + 2H2O ==> H2 + 2CsOH
You will need to add the states depending upon the definitions given for SATP conditions.
Use PV = nRT and solve for n = number of moles. Using the coefficients in the balanced equation, convert moles H2 to moles Cs. Finally, using moles = grams/molar mass, convert moles Cs to grams Cs.
You will need to add the states depending upon the definitions given for SATP conditions.
Use PV = nRT and solve for n = number of moles. Using the coefficients in the balanced equation, convert moles H2 to moles Cs. Finally, using moles = grams/molar mass, convert moles Cs to grams Cs.
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