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4 years ago

How much heat in joules in needed to raise the temperature of 257g of ethanol c of ethanol =2.4j/gC by 49.1?

Chemistry

1 answer:

strojnjashka [21]4 years ago

6 0

Answer:

30284.88J

Explanation:

c=mCtetha

c=257×2.4×49.1

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Answer:

transmission

Explanation:

When light waves passes straight through an object, it is called transmission.

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4 years ago

Read 2 more answers

Bromine (Br2) is produced by reacting HBr with O2, with water as a byproduct. The O2 is part of an air (21 mol % O2, 79 mol % N2

Karolina [17]

Answer:

The mole fractions:

$x_{HBr}=\frac{100mol}{318.5}=0.314$

$x_{Br_2}=\frac{78mol}{318.5}=0.245$

$x_{H_2O}=\frac{78mol}{318.5}=0.245$

$x_{O_2}=\frac{62.5mol}{318.5}=0.196$

Explanation:

The reaction described is:

$2 HBr (g) + 1/2 O_2 (g) \longrightarrow Br_2 (g) + H_2O (g)$

The limiting reactant is the HBr (oxygen is in excess).

a) The mass (in moles) balance for this sistem:

$n_{Br_2}=\frac{ 1 mol Br_2}{1 mol HBr} *n_{HBr}*0.78$

(the 0.78 is because of the fractional conversion)

$n_{O_2}=\frac{ 0.5 mol O_2}{1 mol HBr} *n_{HBr}*1.25$

(the 1.25 is because of the oxygen excess)

$n_{H_2O}=\frac{ 1 mol H_2O}{1 mol Br_2} *n_{Br_2}$

There is only one degree of freedom in this sistem, you can either deffine the moles of HBr you have or the moles of Br2 you want to produce. The other variables are all linked by the equations above.

b) Base of calculation 100 mol of HBr:

$nn_{HBr}=100 mol HBr$

$n_{Br_2}=\frac{ 1 mol Br_2}{1 mol HBr} *100mol HBr*0.78$

$n_{Br_2}=78 mol Br2$

$n_{O_2}=\frac{ 0.5 mol O_2}{1 mol HBr} *100 mol HBr*1.25$

$n_{O_2}=62.5 mol O_2$

$n_{H_2O}=n_{Br_2}= 78 mol$

$n_{total}=(78+78+100+62.5)mol= 318.5mol$

The mole fractions:

$x_{HBr}=\frac{100mol}{318.5}=0.314$

$x_{Br_2}=\frac{78mol}{318.5}=0.245$

$x_{H_2O}=\frac{78mol}{318.5}=0.245$

$x_{O_2}=\frac{62.5mol}{318.5}=0.196$

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3 years ago

the empirical formula of a compound is NO2. it's molecular mass is 92g/mol. What is its molecular formula?

lesantik [10]

The molecular formula:
$N_x(O_2)_x$

$M_{N_x(O_2)_x}=x \times M_N + x \times 2 \times M_O \\ \\
m_N=14 \ \frac{g}{mol} \\
m_O=16 \ \frac{g}{mol} \\ M_{N_x(O_2)_x}=92 \ \frac{g}{mol} \\ \\
92=x \times 14+x \times 2 \times 16 \\
92=14x+32x \\
92=46x \\
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x=2 \\ \\
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The molecular formula is N₂O₄.

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A strong electrolyte is completely ionized. Ex: NaCl --h2o--> Na^+(aq) + Cl^-(aq)

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3 years ago