A compound is found to contain 24.0 g carbon, 4.00 mol hydrogen and 1.204 × 1024 atoms of oxygen. What is the empirical formula of this compound?
Question
Solution 1
To find the empirical formula of the compound, we need to convert the given amounts of carbon, hydrogen, and oxygen into moles.
- For carbon, we know that the molar mass of carbon (C) is approximately 12.01 g/mol. So, we can convert the given mass of carbon into moles by dividing the mass by the Knowee AI is a powerful AI-powered study tool designed to help you to solve study problem.
Knowee AI is a powerful AI-powered study tool designed to help you to solve study problem.
Knowee AI is a powerful AI-powered study tool designed to help you to solve study problem.
Knowee AI is a powerful AI-powered study tool designed to help you to solve study problem.
Knowee AI is a powerful AI-powered study tool designed to help you to solve study problem.
Knowee AI
Similar Questions
A compound has 40% Carbon 6.6% Hydrogen & 53.3% Oxygen. Calculate the Empirical Formula of the compound.
An unknown compound was decomposed into 316 g carbon, 26.3 g hydrogen, and 208 g oxygen. What is its empirical formula?
an organic compound has relative moleculaf mass of 150 and contains 72.0% carbon, 6.67% hydrogen and 21.33% oxygen.Determine the emphirical formula
A 4.235 g sample of a hydrocarbon was burned in oxygen to give 3.810 g of H2O and 13.96 g of CO2. What is the empirical formula of the compound?
a compound composed of only carbon and hydrogen contains these elements in a mass ratio C:H of 0.375. what's the empirical formula
Upgrade your grade with Knowee
Get personalized homework help. Review tough concepts in more detail, or go deeper into your topic by exploring other relevant questions.