All categories

2 years ago

When does a chemical reaction end?

Chemistry

2 answers:

olga nikolaevna [1]2 years ago

6 0

Answer:

When all the reactants end up in the products - when no new atoms can be destroyed or created

Taya2010 [7]2 years ago

3 0

Information: Chemical reactions, in which chemical bonds are broken and formed, require an initial investment of energy. Kinetic energy, the energy of matter in motion, fuels the collisions of atoms, ions, and molecules that are necessary if their old bonds are to break and new ones to form. All molecules store potential energy, which is released when their bonds are broken.

Four forms of energy essential to human functioning are: chemical energy (which is stored and released as chemical bonds are formed and broken), mechanical energy (which directly powers physical activity), radiant energy (emitted as waves such as in sunlight), and electrical energy, the power of moving electrons.

Answer: Chemical reactions begin with reactants and end with products. Synthesis reactions bond reactants together, a process that requires energy, whereas decomposition reactions break the bonds within a reactant and thereby release energy.

You might be interested in

If a cold piece of metal is added to hot water, the water will

Roman55 [17]

Answer:

Over time the metal will cool and the water will heat up. Eventually the two objects will have the same temperature

Explanation:

5 0

3 years ago

Plant Cell

musickatia [10]

Answer:

it's the chloroplast but I'm not sure which on is it it might be the F.

6 0

3 years ago

Solids we need to live

gogolik [260]

Foods are a solid we need to survive

6 0

4 years ago

2. Carbon-11 is a radioactive isotope of carbon. Its half-life is 10 minutes.

Annette [7]

It’s probably probably 01/16 because of the other number don’t make sense except that one

5 0

3 years ago

The combustion of acetylene gas is represented by this equation: 2C2H2(g) + 5O2(g) → 4CO2(g) + 2H2O(g)

MAVERICK [17]

Answer:

Approximately $2.46\; \rm mol$ .

Explanation:

Make use of the molar mass data ( $M({\rm C_2H_2}) = 26.04\; \rm g \cdot mol^{-1}$ ) to calculate the number of moles of molecules in that $64.0\; \rm g$ of $\rm C_2H_2$ :

$\begin{aligned}n({\rm C_2H_2}) &= \frac{m({\rm C_2H_2})}{M} \\ &= \frac{64.0\; \rm g}{26.04\; \rm g\cdot mol^{-1}}\approx 2.46\; \rm mol\end{aligned}$ .

Make sure that the equation for this reaction is balanced.

Coefficient of $\rm C_2H_2$ in this equation: $2$ .

Coefficient of $\rm H_2O$ in this equation: $2$ .

In other words, for every two moles of $\rm C_2H_2$ that this reaction consumes, two moles of $\rm H_2O$ would be produced.

Equivalently, for every mole of $\rm C_2H_2$ that this reaction consumes, one mole of $\rm H_2O$ would be produced.

Hence the ratio: $\displaystyle \frac{n({\rm H_2O})}{n({\rm C_2H_2})} = \frac{2}{2} = 1$ .

Apply this ratio to find the number of moles of $\rm H_2O$ that this reaction would have produced:

$\begin{aligned}n({\rm H_2O}) &= n({\rm C_2H_2}) \cdot \frac{n({\rm H_2O})}{n({\rm C_2H_2})} \\ &\approx 2.46\; \rm mol \times 1 = 2.46\; \rm mol\end{aligned}$ .

3 0

3 years ago