What is the empirical formula of a compound that is 27.3% carbon, 9.10% hydrogen and 63.6% nitrogen by mass?

Chemistry

1 answer:

Viefleur [7K]2 years ago

7 0

Explanation:

Mass ratio C : H : N = 27.3 : 9.10 : 63.6

Mole ratio C : H : N = 27.3/12: 9.10/1 : 63.6/14

( Divide the mass ratio by their molar masses to find the ratio between moles)

Mole ratio = 2.275 : 9.10 : 4.54

= 2.275/2.275 : 9.10/2.275 : 4.54/2.275

= 1 : 4 : 2

Answer is CH4N2

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2.00 L of 0.800 M NaNO3 must be prepared from a solution known to be 2.50 M in concentration.How many mL are required? Plus don'

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Answer:

1.36 × 10³ mL of water.

Explanation:

We can utilize the dilution equation. Recall that:

$\displaystyle M_1V_1= M_2V_2$

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Let the initial concentration and unknown volume be M₁ and V₁, respectively. Let the final concentration and required volume be M₂ and V₂, respectively. Solve for V₁:

$\displaystyle \begin{aligned} (2.50\text{ M})V_1 &= (0.800\text{ M})(2.00\text{ L}) \\ \\ V_1 & = 0.640\text{ L} \end{aligned}$

Therefore, we can begin with 0.640 L of the 2.50 M solution and add enough distilled water to dilute the solution to 2.00 L. The required amount of water is thus:
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