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Wewaii [24]
3 years ago
5

Use the problem below to answer the question: How many grams of H2 would be formed if 34 grams of carbon reacted with an unlimit

ed amount of H2O? The reaction is: C + H2O → CO + H2 The equation is balanced. The starting substance is carbon, C. The ending substance is hydrogen, H2. Using the periodic table, find the molecular mass of H2. H2 = g/mole
Chemistry
2 answers:
Pavlova-9 [17]3 years ago
6 0
34g C * ( 1 mol / 12.0107 ) * ( 1 mol H2 / 1 mol C ) * ( <span>2.01588 g / 1 mol H2 ) = 5.70657164028741 g H2 = 5.7 g H2

Convert grams of C to moles of C using the given amount of grams and the molar mass ( 12.0107 g/mol ).

Gather the mole ratio from the coefficients in the balanced equation and multiply by the ratio.

Convert moles of H2 to grams of H2 </span> using the given amount of grams and the molar mass ( 2.01588 g/mol )<span>.

Revise your answer to have the correct number of significant figures. </span>
Aleksandr [31]3 years ago
5 0

<u>Answer:</u> The mass of hydrogen gas formed will be 5.66 g

<u>Explanation:</u>

To calculate the number of moles, we use the formula:

\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}    .....(1)

<u>For Carbon:</u>

Given mass = 34 g

Molar mass = 12 g/mol

Putting values in above equation, we get:

\text{Moles of carbon}=\frac{34g}{12g/mol}=2.83mol

For the given chemical equation:

C+H_2O\rightarrow CO+H_2

By Stoichiometry of the reaction:

1 mole of carbon produces 1 mole of hydrogen gas.

So, 2.83 moles of carbon atom will produce = \frac{1}{1}\times 2.83=2.83mol of hydrogen gas.

Now, to calculate the mass of hydrogen gas, we use equation 1.

Moles of Hydrogen gas = 2.83 mol

Molar mass of hydrogen gas = 2 g/mol

Putting values in equation 1, we get:

2.83mol=\frac{\text{Mass of Hydrogen gas}}{2g/mol}\\\\\text{Mass of Hydrogen gas}=5.66g

Hence, the mass of hydrogen gas formed will be 5.66 g

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83ef0c8
kumpel [21]

Answer:

0.17325 moles per liter per second

Explanation:

For a first order reaction;

in[A] = in[A]o - kt

Where;

[A]= concentration at time t

[A]o = initial concentration

k= rate constant

t= time taken

ln0.5 =ln1 - 2k

2k = ln1 - ln0.5

k= ln1 - ln0.5/2

k= 0 -(0.693)/2

k= 0.693/2

k= 0.3465 s-1

Rate of reaction = k[A]

Rate = 0.3465 s-1 × 0.50 mol/L

Rate = 0.17325 moles per liter per second

5 0
3 years ago
Please help!!
Olegator [25]
Molarity =  Moles/Liter

Use the molecular atomic mass of NaCl to convert from grams to moles.
Molecular mass of NaCl is the sum of its atomic masses. Look at the periodic table to find these. Na is 23 g/mol and Cl is 35.5 g/mol ,
so NaCl = 23 + 35.5 = 58.5 g/mol

multiply to cancel out grams
76 g NaCl * (1mol / 58.5 g NaCl) = 1.3 mol NaCl

over 1 Liter is just 1.3 M NaCl
Hope this helps!
8 0
3 years ago
I need help ASAP!!!!!!!!!!!!!!!!!!!
liraira [26]

last one? don't take my word though

Explanation:

the suns heat is related to nuclear fusion

6 0
2 years ago
How i the ma number of an atom calculated? (1 point)
Bess [88]
Proton plus neutron is the correct answer. Protons and neutrons have a mass of 1 and electrons have a mass of 0. So in order to find the mass of an atom you need to add the number of protons and the number of neutrons.
4 0
1 year ago
A total of 25.0 mL of 0.150 M potassium hydroxide (KOH) was required to neutralize 15.0 mL of sulfuric acid (H2SO4) of unknown c
Kamila [148]
We are told that KOH is being used to completely neutral H₂SO₄ according to the following reaction:

KOH + H₂SO₄ → H₂O + KHSO₄

If KOH can completely neutralize H₂SO₄, then there must be an equal amount of moles of each as they are in a 1:1 ratio:

0.025 L x 0.150 mol/L = .00375 mol KOH

0.00375 mol KOH x 1 mole H₂SO₄/1 mole KOH = 0.00375 mol H₂SO₄

We are told we have 15 mL of H₂SO₄ initially, so now we can find the original concentration:

0.00375 mol / 0.015 L = 0.25 mol/L

The concentration of H₂SO₄ being neutralized is 0.25 M.
6 0
3 years ago
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