For the following chemical reaction, given 2.5 gram mgso4 with an excess of ba(no3)2, calculate the theoretical mass of baso4 precipitate produced from the reaction (in grams). the following conceptual plan is designed to you convert the mass of the limiting reactant (mgso4) to the mass of the desired product (baso4).

The answer to your question is:  4.9 g of BaSO4

Explanation:

Data

MgSO4 = 2.5 g

Ba(NO3)2 = excess reactant

BaSO4 = ?

Reaction

                  MgSO4   +    Ba(NO3)2      ⇒     BaSO4   +    Mg(NO3)2

MW MgSO4 = 24 + 32 + 64

                    = 120 g

MW BaSO4 = 137 + 32 + 64

                    = 233 g

                  120 g of MgSO4  233g of BaSO4

                  2.5 g                       x

                  x = 4.9 g of BaSO4

radioactive decay occurs in unstable atomic nuclei – that is, ones that don't have enough binding energy to hold

the nucleus together due to an excess of either protons or neutrons.

the ideal gas law equation is as follows

pv = nrt

where p - pressure

v - volume

n - number of moles

r - universal gas constant

t - temperature

so if the pressure, volume and temperature are already known

we are left with n and r

since r is the universal gas constant that has a known fixed value then r too is known

so we are left with 'n'

once we know temperature volume and pressure

we can find the number of moles of gas present using the ideal gas law equation

this is not my own answer, this is an answer for the same question by the user blahblahmali. i do not claim ownership of this account.