The amount of CO that would be required to generate 635 g of CO2 will be 404.14 g
<h3>Stoichiometric problem</h3>
First, let us get the equation of the reaction:
From the equation, we can see that the mole ratio of CO to that of CO2 is 1:1.
635 g of CO2 is to be generated.
Mole of 635 g CO2 = mass/molar mass = 635/44.01 = 14.43 moles
Thus, the equivalent mole of CO required will also be 14.43 moles.
Mass of 14.43 moles CO = moles x molar mass = 14.43 x 28.01 = 404.14 g
Hence, 404.14 g of CO will be required to produce 635 g of CO2
More on stoichiometric problems can be found here: brainly.com/question/14465605
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To find molarity use the following formula
molarity= moles/ liters
first, we need to calculate the moles using the grams of NH₃. remember to convert grams to moles, you need the molar mass of the molecule which you can determine by adding the mass of each atom
molar mass of NH₃ = 14.0 + (3 x 1.01)= 17.03 g/ mol
now, let convert grams to moles
17.0 g (1 mol/ 17.03 grams)= .998 moles NH₃
now, we can plug in these values to solve for molarity
molarity= 0.998 mol/ 2.0 Liters= 0.50 M (the answer is a)
Answer:
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Explanation:
Answer: 0.86g/mL
Explanation:
Mass of empty cylinder = 23.731g
Mass of cylinder + liquid = 26.414g
Mass of the liquid = 26.414 — 23.731
= 2.683g
Volume of the liquid = 3.12mL
Density = Mass / volume
Density = 2.683g / 3.12mL
Density = 0.86g/mL
Answer:
1f 3f 5g 1p 2d
Explanation:
There is only 4f and 5f orbitals.
G is not an orbital.
P orbital starts with 2p
D orbital starts with 3d
