In a certain chemical reaction Compound combines with Compound to produce Compound (and no other products). Measurements were taken of the amounts of and present before and after a reaction that produced some : Compound initial amount final amount Calculate the theoretical yield of . Round your answer to the nearest . Suppose the percent yield of in this reaction was . Calculate the actual amount of that was isolated at the end of the reaction. Round your answer to the nearest .

0.8g.

Explanation:

So, in this question we are to calculate for the actual yield of the product, Say C.

Thus, the equation for Determining the percentage yield is given as;

Percentage yield = actual yield/ theoretical yield × 100 (1).

Therefore, from equation one above we can calculate the value for the percentage yield for product C.

A + B > C.

From the given value we have that, before the reaction there are 1.0 g of A and 7.0 g of B, after the reaction; we have 0 gram of A and 5.2 gram of B. That means that A is the limiting reactant. Thus, A Determines the reaction.

Hence, the mass of product C = 1 g = 0.1 × 10^1 grams.

Therefore, using the reaction (1) above;

Percentage yield = actual yield/ theoretical yield × 100.

80 =( actual yield / 0.1 × 10^1 grams ) × 100.

80 × 0.1 × 10^1 grams = 100 × actual yield.

Actual yield = 0.8 g.

it is to be noted that an alpha particle is an helium nucleus. so it contains 2 protons 2 neutrons and has a mass number of 4. when alpha decay particles are ejected from the nucleus it gets transformed into an atom which has atomic number less than 2 and a mass number less than 4.

an equation that could represent alpha decay is radium 226 decay of alpha particle forms radon 222.

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explanation: