1. How many moles are in 3.4 x 10²⁴ molecules of HCl?
if there are 6.022 × 10²³ molecules in 1 mole of HCl
then there are 3.4 × 10²⁴ molecules in X moles of HCl
X = (3.4 x 10²⁴ × 1) / 6.022 × 10²³ = 5.6 moles of HCl
2. How many grams are in 2.59 x 10²³ formula units of Al₂O₃?
if there are 6.022 × 10²³ units in 1 mole of Al₂O₃
then there are 2.59 × 10²³ units in X moles of Al₂O₃
X = (2.59 x 10²³ × 1) / 6.022 × 10²³ = 0.43 moles of Al₂O₃
number of moles = mass / molecular weight
mass = number of moles × molecular weight
mass of Al₂O₃ = 0.43 × 102 = 43.86 g
3. How many grams are in 9.05 x 1023 atoms of silicon?
if there are 6.022 × 10²³ atoms in 1 mole of silicon
then there are 9.05 × 10²³ atoms in X moles of silicon
X = (9.05 x 10²³ × 1) / 6.022 × 10²³ = 1.5 moles of silicon
mass = number of moles × molecular weight
mass of silicon = 1.5 × 28 = 42 g
4. If you had 7.00 moles of PtO₂, how many grams would you have?
mass = number of moles × molecular weight
mass of PtO₂ = 7 × 227 = 1589 g
5.How many moles are in 29.2 L of oxygen gas at STP?
At standard temperature and pressure (STP) we may use the following formula:
number of moles = volume (L) / 22.4 (L / mol)
number of moles of oxygen = 29.2 / 22.4 = 1.3
6. What is the volume (liters) of 75.8 g of N₂ at STP?
number of moles = mass / molecular weight
number of moles of N₂ = 75.8 / 28 = 2.7 moles
At standard temperature and pressure (STP) we may use the following formula:
number of moles = volume (L) / 22.4 (L / mol)
volume = number of moles × 22.4
volume of N₂ = 2.7 × 22.4 = 60.48 L
1. How many moles are in 3.4 x 10²⁴ molecules of HCl?
if there are 6.022 × 10²³ molecules in 1 mole of HCl
then there are 3.4 × 10²⁴ molecules in X moles of HCl
X = (3.4 x 10²⁴ × 1) / 6.022 × 10²³ = 5.6 moles of HCl
2. How many grams are in 2.59 x 10²³ formula units of Al₂O₃?
if there are 6.022 × 10²³ units in 1 mole of Al₂O₃
then there are 2.59 × 10²³ units in X moles of Al₂O₃
X = (2.59 x 10²³ × 1) / 6.022 × 10²³ = 0.43 moles of Al₂O₃
number of moles = mass / molecular weight
mass = number of moles × molecular weight
mass of Al₂O₃ = 0.43 × 102 = 43.86 g
3. How many grams are in 9.05 x 1023 atoms of silicon?
if there are 6.022 × 10²³ atoms in 1 mole of silicon
then there are 9.05 × 10²³ atoms in X moles of silicon
X = (9.05 x 10²³ × 1) / 6.022 × 10²³ = 1.5 moles of silicon
mass = number of moles × molecular weight
mass of silicon = 1.5 × 28 = 42 g
4. If you had 7.00 moles of PtO₂, how many grams would you have?
mass = number of moles × molecular weight
mass of PtO₂ = 7 × 227 = 1589 g
5.How many moles are in 29.2 L of oxygen gas at STP?
At standard temperature and pressure (STP) we may use the following formula:
number of moles = volume (L) / 22.4 (L / mol)
number of moles of oxygen = 29.2 / 22.4 = 1.3
6. What is the volume (liters) of 75.8 g of N₂ at STP?
number of moles = mass / molecular weight
number of moles of N₂ = 75.8 / 28 = 2.7 moles
At standard temperature and pressure (STP) we may use the following formula:
number of moles = volume (L) / 22.4 (L / mol)
volume = number of moles × 22.4
volume of N₂ = 2.7 × 22.4 = 60.48 L
1-Find the molar mass of the substance.
2-H3PO4
3-New atoms are created.
4-The ratios of the number of moles of each substance that react and that are produced.
5-conservation of mass
6-The number of atoms for every element is equal on both sides of the equation.
7-1:1
8-1:03
9-5.50%
1-Find the molar mass of the substance.
2-H3PO4
3-New atoms are created.
4-The ratios of the number of moles of each substance that react and that are produced.
5-conservation of mass
6-The number of atoms for every element is equal on both sides of the equation.
7-1:1
8-1:03
9-5.50%
a) 24.7 mol
b) 790 g
Explanation:
Step 1: Given data
Volume of the chamber (V): 200. LRoom temperature (T): 23 °CPressure of the gas (P): 3.00 atmStep 2: Convert "T" to Kelvin
We will use the following expression.
K = °C + 273.15
K = 23°C + 273.15 = 296 K
Step 3: Calculate the moles (n) of oxygen
We will use the ideal gas equation.
P × V = n × R × T
n = P × V/R × T
n = 3.00 atm × 200. L/(0.0821 atm.L/mol.K) × 296 K = 24.7 mol
Step 4: Calculate the mass (m) corresponding to 24.7 moles of oxygen
The molar mass (M) of oxygen ga sis 32.00 g/mol. We will calculate the mass of oxygen using the following expression.
m = n × M
m = 24.7 mol × 32.00 g/mol = 790 g
a) 24.7 mol
b) 790 g
Explanation:
Step 1: Given data
Volume of the chamber (V): 200. LRoom temperature (T): 23 °CPressure of the gas (P): 3.00 atmStep 2: Convert "T" to Kelvin
We will use the following expression.
K = °C + 273.15
K = 23°C + 273.15 = 296 K
Step 3: Calculate the moles (n) of oxygen
We will use the ideal gas equation.
P × V = n × R × T
n = P × V/R × T
n = 3.00 atm × 200. L/(0.0821 atm.L/mol.K) × 296 K = 24.7 mol
Step 4: Calculate the mass (m) corresponding to 24.7 moles of oxygen
The molar mass (M) of oxygen ga sis 32.00 g/mol. We will calculate the mass of oxygen using the following expression.
m = n × M
m = 24.7 mol × 32.00 g/mol = 790 g
Answer:
AStep-by-step explanation:
The input force is 50 N. But it will not create not any change. No mechanical advantage is observed.
It will provide an instant answer!