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2 years ago

What happens if you put sugar in someone's gas tank?

1 answer:

4 0

The sugar reacts with the gas, turning it to a semi-solid and sticky substance; clogging the gas lines along with many other things.

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When iron rusts in air iron3 oxide is produced. How many moles of oxygen react with 28.0 mol of iron in the rusting reaction 4fe

Marrrta [24]

This the balanced equation based on the question $4Fe + 3O_2 -\ \textgreater \ 2Fe_2O_3$ .

We then proceed with the following calculations

$28.0molFe*(\frac {3molO_2}{4mol Fe})= 21molO_2$

The answer is $21molO_2$ is produced.

5 0

2 years ago

Is this sentence true or false ? hydrogen is considered to be a metal

victus00 [196]

It is false, hope this helps!

4 0

2 years ago

Read 2 more answers

PLEASE HELP! Count the total number of atoms in H 2 O: 2 3 4 5 6

Darya [45]

3
two hydrogen and 1 oxygen

8 0

2 years ago

Read 2 more answers

Given these reactions, X ( s ) + 1 2 O 2 ( g ) ⟶ XO ( s ) Δ H = − 668.5 k J / m o l XCO 3 ( s ) ⟶ XO ( s ) + CO 2 ( g ) Δ H = +

qwelly [4]

Answer: The $\Delta H^o_{rxn}$ for the reaction is -1052.8 kJ.

Explanation:

Hess’s law of constant heat summation states that the amount of heat absorbed or evolved in a given chemical equation remains the same whether the process occurs in one step or several steps.

According to this law, the chemical equation is treated as ordinary algebraic expressions and can be added or subtracted to yield the required equation. This means that the enthalpy change of the overall reaction is equal to the sum of the enthalpy changes of the intermediate reactions.

The given chemical reaction follows:

$X(s)+\frac{1}{2}O_2(g)+CO_2(g)\rightarrow XCO_3(s)$ $\Delta H^o_{rxn}=?$

The intermediate balanced chemical reaction are:

(1) $X(s)+\frac{1}{2}O_2(g)\rightarrow XO(s)$ $\Delta H_1=-668.5kJ$

(2) $XCO_3(s)\rightarrow XO(s)+CO_2$ $\Delta H_2=+384.3kJ$

The expression for enthalpy of the reaction follows:

$\Delta H^o_{rxn}=[1\times \Delta H_1]+[1\times (-\Delta H_2)]$

Putting values in above equation, we get:

$\Delta H^o_{rxn}=[(1\times (-668.5))+(1\times (-384.3))=-1052.8kJ$

Hence, the $\Delta H^o_{rxn}$ for the reaction is -1052.8 kJ.

7 0

2 years ago

Which of the following is true regarding a voltaic (or galvanic) cell? a) It can only be used with hydrogen. b) It produces elec

N76 [4]

Answer:

b) It produces electrical current spontaneously.

Explanation:

Cells capable of converting chemical energy to electrical energy and vice versa are termed Electrochemical cells. There are two types of electrochemical cells viz: Galvanic or Voltaic cells and Electrolytic cells. Voltaic cell is an elctrochemical cell capable of generating electrical energy from the chemical reaction occuring in it.

The voltaic cell uses spontaneous reduction-oxidation (redox) reactions to generate ions in a half cell that causes electric currents to flow. An half cell is a part of the galvanic cell where either oxidation or reduction reaction is taking place. Hence, the spontaneous production of electric currents is true about Voltaic/Galvanic cells.

3 0

2 years ago