Unbalanced equation 1. Given the following reaction: Si (s) + CI 2(g 35g SICI4 (1) ?g 56g When 56g of silicon are combined with 35g of chlorine gas in a reaction vessel: Smee CI has the Smallect value,it wi be the a. What is the limiting reactant? Chlenhe e lmiting ieachant b. How many moles of the excess reactant are left?

n4 of 14 Consider the following reaction. heat 2 Fe, O, (s) + 3 C(s) → 4 Fe(s) + 3 CO,(g) 3. Calculate the number of grams of Fe,O, needed to react with 11.0 g C. Gmages mass of Fe, O,:

[References] TUTOR Chemical Equations: Gram/Gram Calculation Consider the reaction: SOe) + H;O(1) → H3SO;( Given an initial mass of 15.3 g SO, an excess of H50, and assuming that all of the reactant is converted to product(s), and none is lost, calculate the mass (g) of H7SO3 produced by the reaction.

a piece of zn metal (25)g reacts with 100ml of a 2m hcl solution to form zncl2 and h2 gas. What mass of H2 will be produced if the limitng reagant is fully consumed? How many moles of limiting reagant remains after the reatioin?

For the given Chemical equation, find the number of moles of propionic acid (C;H,O2) and CO, using the number of moles given in the table below. C;H,O; + H2 +02 CH,O4 + C,H4O2 + C;H,O2 + CO2 Fermentation Product Moles Succinic acid (succinate) C4HGO4 Acetic acid (acetate) CH4O2 Carbon dioxide CO2 Hydrogen H2 Propionic acid (propionate) C;HO2 6 12 - 8 y Pyruvic acid (pyruvate) C;H4O; Охуgen (O,) 20

conside ne comDUSuON OT memane. CH.(g) +202(g)→ CO,(g) + 2H,0(g) Suppose 2.o mol of methane are allowed to react with 3.9 mol of oxygen. Part A What is the limiting reagent? methane Previous Answèrs v Correct Part B How many moles of CO, can be made from th s reaction? mol CO,

How many grams of N2 are needed to completely (stoichiometrically) react with 222 g of Br2 ? N2 + 3 Br2 2 NB13 + 44.0 kJ The molar mass of Br2 is g and the molar mass of N2 is mol Br2 (2.22 x 102 g Br2)(- mol Br2 g Br2 mol N2 mol Br2 (-- -) = mol N2 mol Br2 g N2 mol N2 (-- -) = |v g N2 mol N2 а. 1 b. 2 С. 3 d. 4 е. 5 f. 253.719 g. 3.38 х 100 h. 3.26 x 103 i. 44.0 j. 1.33 x 102 k. 9.77 x 103 I. 4.44 x 102 m. 6.66 x 10² n. 500.0 o. 556 р. 90.0 q. 3.2852 r. 159.81 s. 28.013 t. 1.750 u. 0.8750 v. 13.0 w. 0.46306 х. 1.3892 у. 24.5 z. 38.5 аа. 2.190 bb. evolved Cc. absorbed dd. exothermic ee. endothermic

Please explain 5a, c , and d Thank you

a laccd sign in - Search ||| tab hift T 0 caps lock % esc O CHEMICAL REACTIONS Percent yield of chemical reactions Be sure your answer has the correct number of significant digits in it. Explanation K- →1 V Liquid octane (CH₂(CH₂) CH₂) reacts with gaseous oxygen gas (0₂) to produce gaseous carbon dioxide (CO₂) and gaseous water (H₂O). If 10.9 g of water is produced from the reaction of 27.41 g of octane and 176.6 g of oxygen gas, calculate the percent yield of water. m X ? https://www-awu.aleks.com/alekscgi/x/Isl.exe/1o_u-IgNslkr7j8P3jH-IvUrTNdLZh5A8CnG03PBGuXr8iCPa7ZMmym Type here to search A 2 Z P Check ALEKS W S # X * 3 X alt E *** f4 $ D 70 4 C X R % 100 Mc Graw He f6 T V McGraw-Hill Education Campus X 4- G (0) 17 B Y ♫+ & 7 H no f8 © 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Access a ? KAA * J A ALEKS-Shushanik Babayan - Le X + 96sW-8PcvpF38ZsC... A N fg 3 K f10 0/5 L f12 93°F insert alt Shush 11 prt sc ] bac pause ctri

Balance the following chemical reaction, and complete the stoichiometry problem: