Balancing Chemical Equations Quiz

Adjusting coefficients in a chemical equation to ensure the same number of atoms of each element are present on both sides of the equation.

The amount of a substance measured in moles, directly related to the number of molecules.

The amount of a substance produced from a reaction, quantifiable in moles.

The ratio between the moles of one reactant or product to the moles of another.

The number of atoms or molecules in one mole of a substance (approximately 6.022 x 10^23).

The calculation of reactants and products in a chemical reaction using mole ratios from the balanced equation.

Adjusting the coefficients in a chemical equation to ensure equal number of atoms of each element on each side of the equation, e.g. N2 + 3F2 → 2NF3.

Using the given amounts (moles) of one substance in a balanced chemical reaction to determine the moles of another substance involved in the reaction, applying the mole ratio.

Using Avogadro's Number to convert moles of a substance into molecules.

A chemical reaction where gallium bromide interacts with sodium sulfite to yield gallium sulfite and sodium bromide. This chemical reaction has a definite stoichiometry.

In a chemical reaction, tin(II) oxide reacts with nitrogen trifluoride, creating tin(II) fluoride and dinitrogen trioxide.

Adjusting the coefficients in a chemical equation to have an equal number of atoms of each element on both sides of the equation. Example: N2 + 3F2 → 2NF3

If 3.5 moles of Nitrogen react, then 7 moles of Nitrogen Trifluoride will be produced given the balanced chemical equation N2 + 3F2 → 2NF3

0.102 moles of Fluorine will react with 0.034 moles of Nitrogen, based on the mole ratio from the balanced equation.

The mole ratio between nitrogen and nitrogen trifluoride in the reaction N2 + 3F2 → 2NF3 is 1:2

Given that 0.00901 moles of oxygen reacts with excess hexane, 0.00901 moles of water will be produced (assuming excess of hexane and no other factors), based on the balanced reaction.

0.00901 moles of water contain approximately 5.42 x 10^21 molecules, using Avogadro's number.

Balancing the equation HBr + KHCO3 → H2O + KBr + CO2. This yields HBr + KHCO3 → H2O + KBr + CO2 using correct coefficients

6.70 moles of potassium bicarbonate will produce 6.70 moles of carbon dioxide, based on the balanced equation.

From 0.45 moles of HBr with excess KHCO3, approximately 0.45 moles of water is produced, based on the balanced chemical equation.

3Na₂SO₃ + 2GaBr₃ → 3NaBr + Ga₂(SO₃)₃, representing the balanced reaction.

If 70.9 moles of sodium sulfite react, 106.35 moles of sodium bromide are created

Approx. 6.45 x 10^25 molecules of Sodium Bromide are created (70.9 Moles x 6.02 x 10²³).

SnO + 3NF3 → SnF2 + N2O3

2.3 x 10⁻³ moles of Tin (II) oxide require 6.9 x 10⁻³ moles of Nitrogen Trifluoride

Producing 7.02 x 10²⁴ molecules of nitrogen trifluoride needs 1.17 x 10⁻³ moles of SnO

Adjust the coefficients in the chemical equation N2 + F2 → NF3 to have equal numbers of each atom on both sides of the equation.

Calculate the moles of nitrogen trifluoride (NF3) produced when 3.5 moles of nitrogen (N2) react, given the balanced equation.

Determine the moles of fluorine (F2) required to react with 0.034 moles of nitrogen (N2), based on the balanced equation.

Calculate the moles of nitrogen trifluoride (NF3) produced when 0.034 moles of nitrogen (N2) reacts, given the balanced equation.

Convert the moles of NF3 to the number of molecules using Avogadro's number.

Adjust the coefficients in the chemical equation C6H10 + O2 → CO2 + H2O to have equal numbers of each atom on both sides of the equation.

Calculate the moles of water (H2O) produced when 0.00901 moles of oxygen (O2) react with excess hexane (C6H10).

Convert moles of water to molecules using Avogadro's number.

Adjust coefficients in HBr + KHCO3 → H2O + KBr + CO2 to equal the number of atoms on each side of the equation.

Calculate moles of CO2 produced from 6.70 moles of KHCO3, given the balanced equation in the reaction.

Calculate moles of H2O produced when 0.45 moles of HBr reacts with excess KHCO3, based on the balanced equation.

Determine the coefficients to balance the reaction: 3Na₂SO₃ + 2GaBr₃ → 3NaBr + Ga₂(SO₃)₃

Calculate the moles of NaBr produced when 70.9 moles of Na₂SO₃ react, based on the balanced reaction.

Determine the number of NaBr molecules produced from 70.9 mole of Na₂SO₃, utilizing the balanced chemical equation and Avogadro's number.

Determine correct coefficients to balance SnO + NF3 → SnF2 + N2O3

Calculate moles of NF3 required to react with 2.3 x 10⁻³ moles of SnO, considering the balanced equation for SnO + NF3 reaction.

Calculate moles of SnO required to produce 7.02 x 10²⁴ molecules of NF3, based on the balanced reaction between Tin (II) oxide and Nitrogen Trifluoride.