CBSE11•MCQs
+4-1
In the reaction N2(g) + 3H2(g) → 2NH3(g), if 17.86 x 10^2 mol of N2 and 4.96 x 10^3 mol of H2 are available, how much NH3 (in moles) can be formed?
Choose an option
Related Questions
View all →Proust's work with natural and synthetic samples of cupric carbonate showed identical percentage compositions of copper,
CBSE11
Despite its successes, Dalton's Atomic Theory failed to explain which two phenomena?
CBSE11
Given carbon isotopes: 12C (98.892%, 12 u), 13C (1.108%, 13.00335 u), and 14C (2x10^-10%, 14.00317 u). What is the calcu
CBSE11
A compound has a molar mass of 98.96 g/mol and its percentage composition is 4.07% H, 24.27% C, and 71.65% Cl. Determine
CBSE11
Calculate the mass of water (in g) produced by the combustion of 16 g of methane (CH4). (CH4 + 2O2 → CO2 + 2H2O; Atomic
CBSE11
How many moles of methane (CH4) are required to produce 22 g of CO2 after combustion? (CH4 + 2O2 → CO2 + 2H2O; Atomic ma
CBSE11
If 10 volumes of dihydrogen gas reacts with 5 volumes of dioxygen gas, how many volumes of water vapour would be produce
CBSE11
What is the mass per cent of carbon in ethanol (C2H5OH)? (Atomic masses: C=12.01, H=1.008, O=16.00)
CBSE11
More from CBSE11
View all →Proust's work with natural and synthetic samples of cupric carbonate showed identical percentage compositions of copper,
CBSE11
Despite its successes, Dalton's Atomic Theory failed to explain which two phenomena?
CBSE11
Given carbon isotopes: 12C (98.892%, 12 u), 13C (1.108%, 13.00335 u), and 14C (2x10^-10%, 14.00317 u). What is the calcu
CBSE11
A compound has a molar mass of 98.96 g/mol and its percentage composition is 4.07% H, 24.27% C, and 71.65% Cl. Determine
CBSE11
Calculate the mass of water (in g) produced by the combustion of 16 g of methane (CH4). (CH4 + 2O2 → CO2 + 2H2O; Atomic
CBSE11
How many moles of methane (CH4) are required to produce 22 g of CO2 after combustion? (CH4 + 2O2 → CO2 + 2H2O; Atomic ma
CBSE11
Practice Other NCERT Exams
Practice More CBSE11 Questions
Explore more questions and study resources