54.54 moles
ca
54.54
44.01
You first have to find how many moles of CO2 you have so you find its molar mass, (Carbon=12 Oxygen = 16(2)) then you add 12+32 to get the molar mass which is 44 you should also be given a mass, of how much CO2 there is.. or else you cannot calculate the moles. moles are mass/molar mass once you get the moles just multiply the number of moles by Avogadros constant (6.02x1023) Say if the mass was 4.56 g of C02 that you had then you just do 4.56/44 = 0.103636363 mol now multiply that by avogadro's constant and you have the number of atoms/particles/formula units
30 moles
Given the balanced equation2C3H8O + 9O2 --> 6CO2 + 8H2OTo find the number of moles CO2 that will be produced from 0.33 mol C3H8O, we must convert from moles to moles (mol --> mol conversion).0.33 mol C3H8O * 6 molecules CO2 = 0.99 mol CO2---------- 2 molecules C3H8O
As one mole of CO2 contain 2 oxygen having molar mass 32. Soo there will be 0.50 moles of CO2 which contain 16g of oxygen....!
number of moles of co2 is 5.6 lit at ntp According to the relation that PV=nRT 760*v=5.6*0.0821*273 V=0.1649
0.75 moles CO2 x 6.02x10^23 molecules/mole = 4.5x10^23 molecules
For this you need the atomic (molecular) mass of CO2. Take the number of grams and divide it by the atomic mass. Multiply by one mole for units to cancel. CO2=44.0 grams454 grams CO2 / (44.0 grams) = 10.3 moles CO2
calculate the number of moles of carbon and of the other and by number of moles you can proceed further. the next step is that you divide by the smallest ratio. hence obtaining your empirical formula.
12×1023 molecules
44.01
The number of molecules is 0,90332112855.10e23.
You first have to find how many moles of CO2 you have so you find its molar mass, (Carbon=12 Oxygen = 16(2)) then you add 12+32 to get the molar mass which is 44 you should also be given a mass, of how much CO2 there is.. or else you cannot calculate the moles. moles are mass/molar mass once you get the moles just multiply the number of moles by Avogadros constant (6.02x1023) Say if the mass was 4.56 g of C02 that you had then you just do 4.56/44 = 0.103636363 mol now multiply that by avogadro's constant and you have the number of atoms/particles/formula units
Knowing what the answer options are is important for a person to know which is correct. It would be helpful to provide the answer choices as well.
CO2 + 4H2 --> CH4 + 2H2O0.500 moles CO2 (1 mole CH4/1 mole CO2) = 0.500 moles CH40.500 moles CO2 (2 moles H2O/1 mole CO2) = 1.00 moles H2O-------------------------------------------------------------------------------------add= 1.50 moles total product====================
First write the balance equation: Na2CO3 + 2HNO3 ==> 2NaNO3 + CO2 + H2O Next calculate moles of Na2CO3 used: 7.5 g x 1 mole/106 g = 0.071 moles Na2CO3 Then look at mole ratio of Na2CO3 to CO2 and see that it is 1 to 1 Thus, moles CO2 produced = 0.071 moles Finally, convert moles CO2 to grams of CO2: 0.071 moles x 44g/mole = 3.1 g (to 2 significant figures)
To determine the number of liters of carbon dioxide produced in this reaction, we need the balanced equation and the molar mass of carbon dioxide. The balanced equation is: CaCO3 + 2HCl → CaCl2 + CO2 + H2O The molar mass of CO2 is 44.01 g/mol. First, we calculate the number of moles of CaCO3: 906 g / molar mass of CaCO3 = moles of CaCO3 Using the balanced equation, we see that the stoichiometric coefficient of CO2 is 1. This means that the number of moles of CO2 produced is equal to the number of moles of CaCO3. Finally, we convert moles of CO2 to liters using the ideal gas law: moles of CO2 x 22.4 L/mol = liters of CO2. Therefore, the number of liters of CO2 produced from 906 grams of CaCO3 can be calculated as follows: liters of CO2 = (906 g / molar mass of CaCO3) x 22.4 L/mol