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If 5.0 moles of NH3 are produce how many moles of N2 must have been used?
If 5.0 moles of NH3 are produced 2.5 moles of N2 are used.
What mass of NH3 is produced when 1.20 mol of N2 react completely in the following equation N2 plus 3H2 2NH3?
N2 + 3H2 ==> 2NH3moles N2 = 1.20 molesmoles NH3 formed = 1.20 moles N2 x 2 moles NH3/1 moles N2 = 2.40 moles NH3mass NH3 = 2.40 moles x 17 g/mole = 40.8 g NH3
How many moles of N2 are in 50g of it?
To determine the number of moles of N2 in 50g, you first need to find the molar mass of N2 (28.02 g/mol). Then, you divide the given mass (50g) by the molar mass to get the number of moles. In this case, 50g / 28.02 g/mol ≈ 1.79 moles of N2.
Calculate the mass grams of N2 gas required to occupy a 3.0 mL container at 100 C and 0.914 ATM and explain how you did it?
Use equation n=PV/RT where n is number of moles and R is gas constant. Use R= .8314 L-Atm/mol-K. convert 3 ml to liters(3/1000) and 100C to Kelvin (100+273) and solve for moles. Convert moles to grams. 1 mol of N2 equals 28 grams
Find the mass in grams of 4.00x1023 molecules of N2?
1 mole N2 = 28.0134g 1 mole N2 = 6.022 x 1023 molecules N2 28.0134g N2 = 6.022 x 1023 molecules N2 (4.00 x 1023 molecules N2) x (28.0134g/6.022 x 1023 molecules) = 18.6g N2
How many grams of nitrogen are required to react with 2.79 g of hydrogen to produce ammonia?
In the reaction 3H2 + N2 --> 2NH3, the ratio of H2 to N2 is 3:1. To calculate the amount of N2 required, we need to first convert the mass of H2 to moles, then use the ratio to find the moles of N2 needed, and finally convert the moles of N2 to grams. After the calculation, we find that 2.79 g of H2 requires 3.31 g of N2 to react completely.
How many moles of nitrogen are required to convert 9 mol hydrogen gas to ammonia gas?
The balanced chemical equation for the reaction between nitrogen and hydrogen to produce ammonia is: 3 H2 + N2 -> 2 NH3 From the balanced equation, we see that 1 mole of N2 produces 2 moles of NH3. Therefore, to convert 9 moles of H2 to NH3, we would need 9/3 = 3 moles of N2.
How many moles of nitrogen are needed to convert 9.0 mol hydrogen gas to ammonia gas?
The balanced chemical equation for the reaction is: N2 + 3H2 -> 2NH3. This means that 1 mole of N2 reacts with 3 moles of H2 to produce 2 moles of NH3. Therefore, to convert 9.0 mol of H2, you would need 9.0/3 = 3.0 moles of N2.
If 5.0 moles of NH3 are produce how many moles of N2 must have been used?
If 5.0 moles of NH3 are produced 2.5 moles of N2 are used.
What is mass of N2 required to occupy 3.0 L at 100C and 700 mmHg?
To find the mass of N2, first calculate the moles of N2 using the ideal gas law: PV = nRT. Then use the molar mass of N2 to convert moles to grams. Given that the volume is 3.0 L, the temperature is 100°C (373 K), and the pressure is 700 mmHg (93.3 kPa), you can substitute these values into the ideal gas law to find the moles of N2.
What mass of NH3 is produced when 1.20 mol of N2 react completely in the following equation N2 plus 3H2 2NH3?
N2 + 3H2 ==> 2NH3moles N2 = 1.20 molesmoles NH3 formed = 1.20 moles N2 x 2 moles NH3/1 moles N2 = 2.40 moles NH3mass NH3 = 2.40 moles x 17 g/mole = 40.8 g NH3
How many moles of H2are needed to react with 0.90moles N2?
Assuming a balanced chemical equation, you would need 3 moles of H2 to react with 1 mole of N2. Therefore, if you have 0.90 moles of N2, you would need 0.90 x 3 = 2.70 moles of H2 to fully react with it.
How many moles of nitrogen are needed to convert 9.0 mole hydrogen gas to ammonia gas?
To form ammonia, balanced reaction is N(2) + 3H(2) ---> 2NH(3) + H(2)O. As you can see for 1 mole of nitrogen three moles of hydrogen is required. Hence for your question, 3 moles nitrogen is required to satisfy the ratio.
How do you find if you have 14.5 moles of N2 how many moles of H2 are theoretically needed to produce 22.5 moles of NH3 according to the reaction N2 plus 3H2 2NH3?
N2 + 3H2 -> 2NH3 If you have moles produced you can do it this way. 22.5 moles NH3 (3 moles H2/2 moles NH3) = 33.8 moles H2 needed -----------------------------------
How many moles of N2 reacted if 0.40 mole NH3 is produced?
2 x 0.60 = 1.2 the reaction is N2 + 3H2 -> 2NH3 (1 mole of nitrogen N2 give 2 moles of NH3)
How many moles of N2 are in 50g of it?
To determine the number of moles of N2 in 50g, you first need to find the molar mass of N2 (28.02 g/mol). Then, you divide the given mass (50g) by the molar mass to get the number of moles. In this case, 50g / 28.02 g/mol ≈ 1.79 moles of N2.
How many moles of N2 are ina 400.0ml container at 780 mm Hg and 135 degree Celsius?
To find the moles of N2, we need to use the ideal gas law equation: PV = nRT. First, convert 400.0 mL to liters (0.400 L). Then convert 780 mmHg to atm (0.998 atm), and 135 degrees Celsius to Kelvin (408 K). Plug these values into the equation to solve for n, which gives you the moles of N2 in the container.
