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xz_007 [3.2K]
3 years ago
10

Calculate the mass of 3.5 mol C6H6

Chemistry
1 answer:
Lilit [14]3 years ago
4 0
(3.5mol)(24.106 g/1mol c6h6) =84.371 g C6H6
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How many milliliters of a stock solution of 6.20 M HNO3 would you have to use to prepare 0.130 L of 0.470 M HNO3?
Mandarinka [93]

Answer:

9.85

Explanation:

M1V1 =M2V2

6.20×v1= 0.470×0.130

v1 = ( 0.470 × 0.130 ) ÷ 6.20

v1 = 0.0098 L × 1000

V1 = 9.8 ml

6 0
2 years ago
Research the compositions of Pennies. What was the composition of each of your Pennies prior to treatment
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Answer:

History of composition

Years Material Weight (grains)

1944–1946 gilding metal (95% copper, 5% zinc) 48 grains

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What volume of hydrogen (in L) is produced
scZoUnD [109]

Answer:

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Explanation:

5 0
3 years ago
Consider the reaction:
stich3 [128]

Answer:

\large \boxed{\text{-851.4 kJ/mol}}

Explanation:

2Al(s) + Fe₂O₃(s) ⟶ Al₂O₃(s) + 2Fe(s); ΔᵣH = ?

The formula for calculating the enthalpy change of a reaction by using the enthalpies of formation of reactants and products is

\Delta_{\text{r}}H^{\circ} = \sum \Delta_{\text{f}} H^{\circ} (\text{products}) - \sum\Delta_{\text{f}}H^{\circ} (\text{reactants})

                            2Al(s) + Fe₂O₃(s) ⟶ Al₂O₃(s) + 2Fe(s)

ΔfH°/kJ·mol⁻¹:         0         -824.3         -1675.7         0

\begin{array}{rcl}\Delta_{\text{r}}H^{\circ} & = & [1(-1675.7) + 2(0)] - [2(0) - 1(-824.3)]\\& = & -1675.7 + 824.3\\& = & \textbf{-851.4 kJ/mol}\\\end{array}\\\text{The enthalpy change is } \large \boxed{\textbf{-851.4 kJ/mol}}

7 0
3 years ago
Is Carbon combustible? Why or why not?
valkas [14]
Carbon is not combustible because when it combines with oxygen its energy increases thus it doesnt combust. 
3 0
3 years ago
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