There are two kinds of mixtures which are homogeneous and the heterogeneous. Homogeneous mixtures are mixtures that maintain the same uniform appearance and composition throughout; whereas, heterogeneous mixtures are mixtures that contain different visible substances or phases. Here are examples of each mixture.
Homogeneous mixtures: Rainwater, Air and Dishwashing detergent (This kind of mixture only shows one phase of matter)
Heterogeneous mixtures: cereals with milk, ice in soda and mixed nuts. (Obviously, this kind of mixture contains different phases of matter either in liquid, solid or gas).
Reactants are NaHCO3 and HC2H3O2 because they are on the left side of the arrow, aka they’re what’s going in to make the products. NaC2H3O2, H2O and CO2 are the products bc they’re on the right side of the arrow, aka they are the results of the reactants combining
The total pressure in the container is <u>2.02</u> atm.
<em>Step</em> 1. Calculate the<em> total number of moles.
</em>
Moles of He = 1.00 g He × (1.00 mol He/4.003 g He) = 0.2498 mol He
Moles of F₂ = 14.0 g F₂ × (1 mol F₂/38.00 g F₂) = 0.3684 mol F₂
Moles of Ar = 19.00 g Ar × (1 mol Ar/39.95 g Ar) = 0.4756 mol Ar
<em>Total moles</em> = (0.2498 + 0.3684 + 0.4756) mol = <em>1.094 mol
</em>
<em>Step </em>2. Calculate the <em>total pressure</em>.
Use the <em>Ideal Gas Law</em>: <em>pV = nRT
</em>
We can solve the equation to get the pressure:
<em>p</em> = (<em>nRT</em>)/<em>V</em>
<em>n</em> = 1.094 mol
<em>R</em> = 0.082 06 L·atm·K⁻¹mol⁻¹
<em>T</em> = (20.0 + 273.15) K = 293.15 K
<em>V</em> = 13.0 L
∴ <em>p</em> = (1.094 mol × 0.082 06 L·atm·K⁻¹mol⁻¹ × 293.15 K)/13.0 L = 2.02 atm
<span>a. the reactants to the surroundings.
That is because in an exothermic reaction, energy is being released. </span>