In the following reaction, how many grams of nabr will react with 311 grams of pb(no3)2?
pb(no3)2(aq)+2nabr(g) -> pbbr2(s) + 2nano3(aq)
the molar mass of nabr is 102.9 grams and that of pb(no3)2 is 331.21 grams.

193.4 grams

Explanation: According to avogadro's law, 1 mole of every substance weighs equal to the molecular mass and contains avogadro's number of particles.

To calculate the moles, we use the equation:

According to stoichiometry

1 mole of reacts with 2 moles of

0.94 moles of will react with= of

Mass of

193.24g

Explanation:

Step 1:

The balanced equation for the reaction. This is illustrated below:

Pb(NO3)2(aq) + 2NaBr(g) -> PbBr2(s) + 2NaNO3(aq)

Step 2:

Determination of the masses of Pb(NO3)2 and NaBr that reacted from the balanced equation. This is illustrated below:

Molar Mass of Pb(NO3)2 = 331.21g/mol

Molar Mass of NaBr = 102.9g/mol

Mass of NaBr from the balanced equation = 2 x 102.9 = 205.8g.

From the balanced equation,

Mass of Pb(NO3)2 that reacted = 331.21g

Mass of NaBr that reacted = 205.8g

Step 3:

Determination of the mass of NaBr that reacted with 311g of Pb(NO3)2. This is illustrated below:

From the balanced equation above,

331.21g of Pb(NO3)2 reacted with 205.8g of NaBr.

Therefore, 311g of Pb(NO3)2 will react with = (311x205.8)/331.21 = 193.24g of NaBr.

From the calculations made above, 193.24g of NaBr will react with 311g of Pb(NO3)2

the equation that correctly represent the reaction for formation of ammonia is

n2+ 3h2 → 2nh3 (answer d)

1 mole of nitrogen gas (n2) react with 3 moles of hydrogen gas (h2) to form 2 moles of ammonia ( nh3). this is in a process known as haber process were iron is used as a catalyst and reaction take place that a higher temperature and pressure. the process is exothermic hence energy is released.