Chemistry Answers

$$\ce{2C_4H_{10}(g) +13O_2(g) -> 8 CO_2(g) + 10H_2O(l)}$$

$65cm^3$ of butane is burnt in $65cm^3$ of oxygen. Find the volume of carbon dioxide produced.\

Solution\

Assume\

i) $O_2$ and $CO_2$ are ideal gas at STP condition $22.7dm^3/mol$\

ii) $C_4H_{10}$ is limiting reactant with lowest coefficient in the equation while $O_2$ is the excess reactant.

$n_{O_2 (real)}=0.065/22.7=2.8634\times10^-3$ mol $O_2$(real)

$$From\qquad equation:$$$$\ce{2C_4H_{10}(g) :13O_2(g) }$$

$$Real:$$$$\ce{X C_4H_{10}(g) :(2.8634\times{10^-3}) O_2(g) }$$

Ratio: $\frac{2}{13}=\frac{X}{2.8634\times{10^-3}}$\

$X=\frac{2}{13}\times(2.8634\times{10^-3})=4.4052\times10^-4$ mol $C_4H_{10}(real)$ which is the limiting reactant.

$$From\qquad equation:$$$$\ce{2C_4H_{10}(g) :8CO_2(g) }$$

$$Real:$$$$\ce{4.4052\times10^{-4} C_4H_{10}(g) :Y CO_2(g) }$$

$Y=\frac{8}{2}\times(4.4052\times10^{-4})=1.7621\times10^-3$ mol $CO_2(real)$ 

$V_{CO_2}(real)=1.7621\times10^-3$ mol $\times 22.7dm^3/mol=0.039999dm^3=0.04dm^3=40cm^3$

Correct?

Draw an ion with molecular formula C3H5O6P2- with aldehyde , secondary alcohol and phosphate functional group

Aqueous copper (III) nitrate reacts with aqueous sodium phosphate to form solid copper (III) phosphate

30% HCI solution by mass

What volume of hydrogen sulfide gas is formed at 0°C and 100 kPa when 1.24g iron(II) sulfide is reacted with 30 mL of 1.04 mol L^-1 hydrochloric acid solution? Iron(II) chloride is the other product.

Answer is 0.32 L (2 sf)

Calculate the number of atoms sampled in a 2x2x2,um-cubic in the surface of Nickel

⦁ What is the molarity of a solution that contains 10.0 grams of Silver Nitrate that has been dissolved in 750g of water

⦁ What is the molarity of a solution that contains 10.0 grams of Silver Nitrate that has been dissolved in 750g of water

Silver nitrate + potassium phosphate

7.36x10^22 free oxygen atoms